Final answer:
The hybridization of the central atom in XeF4 is sp3d2, which is determined by the square planar structure and the presence of six electron pairs around the xenon atom, as predicted by the VSEPR model.
Step-by-step explanation:
The hybridization of the central atom in XeF4 is a topic concerning molecular geometry and chemical bonding. According to the Valence Shell Electron Pair Repulsion (VSEPR) model, xenon tetrafluoride (XeF4) has a square planar structure with six electron pairs surrounding the xenon (Xe) atom. Four of these pairs are used in forming bonds with fluorine atoms, and the remaining two are lone pairs.
Given this arrangement, xenon must utilize its d-orbitals in addition to the s and p orbitals to accommodate all electron pairs, leading to a sp3d2 hybridization. The square planar geometry is part of an octahedral electron pair arrangement where two of the positions are occupied by lone pairs. Therefore, the correct hybridization of the central atom in XeF4 is sp3d2, which allows for the necessary orbitals to form the bonds and accommodate the lone pairs.